Vanadium(V) oxide: Difference between revisions

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Chemical compound

3D model of a vanadium(V) oxide monolayer

Vanadium(V) oxide, also known as vanadium pentoxide, is the inorganic compound with the formula V_O_. It is a brown/yellow solid, although when freshly precipitated, it appears orange. Because of its high oxidation state, it is both an amphoteric oxide and an oxidizing agent. It is the most stable compound of vanadium and is used as a catalyst in the production of sulfuric acid and maleic anhydride.

Structure

Vanadium(V) oxide adopts a layered structure consisting of distorted octahedra. Each vanadium center is surrounded by six oxygen atoms, forming a distorted octahedron. The V-O bonds are of different lengths, reflecting the different oxidation states of vanadium in the structure.

Production

Vanadium(V) oxide is produced by the calcination of ammonium metavanadate, NH_VO_. The process involves heating the compound in air, which results in the release of ammonia and water, leaving behind V_O_.

Applications

Vanadium(V) oxide is primarily used as a catalyst in the contact process for the production of sulfuric acid. It is also used in the production of maleic anhydride and as a precursor to other vanadium compounds. Additionally, it is used in ceramics and as a colorant for glass.

Reactions

Vanadium(V) oxide is an oxidizing agent and can be reduced to vanadium(IV) oxide, V_O_, and further to vanadium(III) oxide, V_O_. It reacts with alkalis to form vanadates and with acids to form vanadium oxytrichloride.

Safety

Vanadium(V) oxide is toxic and can cause irritation to the eyes, skin, and respiratory tract. It is important to handle it with care and use appropriate protective equipment.

Related pages

References

Greenwood, N. N.; Earnshaw, A. (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 0-08-037941-9.
Cotton, F. Albert; Wilkinson, Geoffrey (1988). Advanced Inorganic Chemistry (5th ed.). Wiley. ISBN 0-471-84997-9.

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-== Vanadium(V) Oxide ==
+{{short description|Chemical compound}}
+{{Use dmy dates|date=October 2023}}
-Vanadium(V) oxide, also known as vanadium pentoxide or V2O5, is a chemical compound with the formula V2O5. It is a dark brown solid that is commonly used as a catalyst and in the production of various vanadium compounds. Vanadium(V) oxide has several important applications in industry and research.
+[[File:Vanadium-pentoxide-monolayer-3D-balls.png|thumb|right|3D model of a vanadium(V) oxide monolayer]]
+[[File:Vanadium_oxidation_states.jpg|thumb|right|Vanadium oxidation states]]
+[[File:V2O5powder.jpg|thumb|right|Vanadium(V) oxide powder]]
+[[File:V2O5_hydrous.jpg|thumb|right|Hydrous vanadium(V) oxide]]
+[[File:V2O5OxNaphth.svg|thumb|right|Chemical structure of vanadium(V) oxide]]
+[[File:V2o5label.jpg|thumb|right|Label of vanadium(V) oxide]]
-=== Chemical Properties ===
+'''Vanadium(V) oxide''', also known as '''vanadium pentoxide''', is the inorganic compound with the formula V_O_. It is a brown/yellow solid, although when freshly precipitated, it appears orange. Because of its high oxidation state, it is both an amphoteric oxide and an oxidizing agent. It is the most stable compound of vanadium and is used as a catalyst in the production of sulfuric acid and maleic anhydride.
-Vanadium(V) oxide is an inorganic compound composed of vanadium and oxygen. It has a molecular weight of 181.88 g/mol and a melting point of 690°C. The compound is highly soluble in water, forming an acidic solution. It is also soluble in other polar solvents such as ethanol and acetone.
+==Structure==
+Vanadium(V) oxide adopts a layered structure consisting of distorted octahedra. Each vanadium center is surrounded by six oxygen atoms, forming a distorted octahedron. The V-O bonds are of different lengths, reflecting the different oxidation states of vanadium in the structure.
-=== Uses ===
+==Production==
+Vanadium(V) oxide is produced by the calcination of ammonium metavanadate, NH_VO_. The process involves heating the compound in air, which results in the release of ammonia and water, leaving behind V_O_.
-Vanadium(V) oxide is primarily used as a catalyst in the production of sulfuric acid. It helps to convert sulfur dioxide (SO2) into sulfur trioxide (SO3), which is then used to produce sulfuric acid. This process, known as the contact process, is one of the most important industrial applications of vanadium(V) oxide.
+==Applications==
+Vanadium(V) oxide is primarily used as a catalyst in the contact process for the production of sulfuric acid. It is also used in the production of maleic anhydride and as a precursor to other vanadium compounds. Additionally, it is used in ceramics and as a colorant for glass.
-Another significant application of vanadium(V) oxide is in the production of ceramics. It is used as a pigment and a glaze for ceramics, providing a yellow color. Vanadium(V) oxide is also utilized in the manufacturing of glass, where it acts as a colorant and a UV absorber.
+==Reactions==
+Vanadium(V) oxide is an oxidizing agent and can be reduced to vanadium(IV) oxide, V_O_, and further to vanadium(III) oxide, V_O_. It reacts with alkalis to form vanadates and with acids to form vanadium oxytrichloride.
-Furthermore, vanadium(V) oxide finds applications in the field of energy storage. It is used as a cathode material in lithium-ion batteries due to its high energy density and stability. Vanadium(V) oxide-based batteries have the potential to store more energy and have a longer lifespan compared to traditional lithium-ion batteries.
+==Safety==
+Vanadium(V) oxide is toxic and can cause irritation to the eyes, skin, and respiratory tract. It is important to handle it with care and use appropriate protective equipment.
-=== Health and Safety ===
-Vanadium(V) oxide is considered to be a hazardous substance. It can cause irritation to the skin, eyes, and respiratory system upon contact or inhalation. Prolonged exposure to vanadium(V) oxide may lead to lung damage and other health issues. Therefore, proper safety precautions, such as wearing protective clothing and using adequate ventilation, should be followed when handling this compound.
-=== References ===
-<references />
-== See Also ==
+==Related pages==
 * [[Vanadium]]
 * [[Oxide]]
-* [[Catalyst]]
+* [[Catalysis]]
-* [[Sulfuric Acid]]
+* [[Sulfuric acid]]
-* [[Lithium-ion Battery]]
+==References==
+* Greenwood, N. N.; Earnshaw, A. (1997). ''Chemistry of the Elements'' (2nd ed.). Butterworth-Heinemann. ISBN 0-08-037941-9.
+* Cotton, F. Albert; Wilkinson, Geoffrey (1988). ''Advanced Inorganic Chemistry'' (5th ed.). Wiley. ISBN 0-471-84997-9.
-[[Category:Chemical Compounds]]
+[[Category:Vanadium compounds]]
-[[Category:Vanadium Compounds]]
 [[Category:Oxides]]
-[[Category:Catalysts]]
+[[Category:Transition metal oxides]]
-[[Category:Industrial Applications]]
-[[Category:Energy Storage]]